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Lewis structures of acids and bases
1. Draw the Lewis structure of the conjugate base for the following acid: H2SO4. Remember to include charges and non-bonding electrons where necessary. Use an expanded octet on sulfur to minimize formal charges.
2. Draw the conjugate acid for the following base. ::Cl::- Remember to include charges and non-bonding electrons where necessary.
3. Determine the dissociation constants for the following acids. Express the answers in proper scientific notation where appropriate.
Acid PKa KAA 3.0B 8.10C -1.0Which is the strongest acid?
4. Rank the given compounds based on their relative acidities.HF, H2C=CH2, NH3, H3CCH3, HC-=CCH3
Determine how many liters of O 2 gas should be mixed at constant temperature and pressure?
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Compute the pH of the solution before the addition of any HNO3. Kb of NH3 =1.8 × 10-5.
A 155 mL sample of rainwater is titrated using 0.0095 M NaOH solution. If 4.8 mL of the NaOH solution was required to reach the endpoint, what was the pH of the rainwater?
Calculate the work done on a 2500. kg car in accelerating it from rest to a speed of 100. km/hr.
Potassium chloride is used in the kitchen as a salt substitute (in place of sodium chloride). Suppose you were planning to make ice cream but discovered too late that you were out of table salt for making the ice bath.
Standard potentials measured against the standard hydrogen electrode, Standard potentials are measured against the standard hydrogen electrode (S.H.E.). Because it is not always convenient to use a S.H.E
A 0.12M solution of a weak acid HA has pH = 2.49. What is the Ka of this acid.
A power plant burns 10^4 kg hr-1 of coal containing 2.5% sulfur. The effluent is released from a single stack of height 70 m. The plume rise is normally about 30 m.
Equal masses of water and ethylene glycol are mixed. What is the concentration of ethylene glycol in units of molality? The molar mass of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively.
Calculate the pressure difference between CH4 and an ideal gas under these conditions. The van der Waals constants for CH 4 are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.
given 4 NH3(g) + 5 O2(g)4 NO(g) + 6 H2O(g) 1,25g of NH3 reacts with 2,29g of O2 what is the limiting reactant?
3H2 (g) + N2 (g) 2NH3(g), Kc = 6.0 × 10-2 at 500°C for this nitrogen fixation reaction. What is the equilibrium concentration of N2 If 0.250 M H2 and 0.050 M NH3 are present at equilibrium?
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